CHEMISTRY HIGH SCHOOL

What is the mass of 2.50 ×1022 molecules of NaOH (Molar mass = 40.0 g/mol)?

Answers

Answer 1

Answer: Two things are given to us: The "molar mass" of NaOH and the number of molecules of NaOH.

The molar mass is different from "mass"; 1 mole of NaOH is equal to 40.0g/mol.
When the question asks, what is the mass? It is referring to how many grams there are.

First, we are going to convert the molecules to atoms using Avogadro's number (=6.02 x 10^23)

(2.50 x 10^22 molecules) x (6.02 x 10^23 atoms) = 0.042 mol

Next, we are going to convert from moles to grams.

0.042 mol of NaOH x 40.0 g of NaOH/1 mole = 1.68g of NaOH.

There are 1.68 grams in 2.50 x 10^22 molecules of NaOH.

Answer 2

Answer:

Hello!

What is the mass of 2.50 ×1022 molecules of NaOH (Molar mass = 40.0 g/mol)?

Data:

Molar Mass of NaOH = 40 g/mol

Solving: According to the Law Avogradro, we have in 1 mole of a substance, 6.02x10²³ atoms/mol or molecules

1 mol -------------------- 6.02*10²³ molecules

y mol -------------------- 2.50*10²² molecules

$(1)/(y) = (6.02*10^(23))/(0.250*10^(23))$

Product of extremes equals product of means

$6.02*10^(23)*y = 0.250*10^(23)*1$

$6.02*10^(23)\:y = 0.250*10^(23)$

$y = (0.250*10^(23))/(6.02*10^(23))$

$\boxed{y \approx 0.042\:mol}$

Solving: Find the mass value now

40 g ----------------- 1 mol of NaOH

x g ------------- 0.042 mol of NaOH

$x = 40*0.042$

$\boxed{\boxed{x = 1.68\:g}}\end{array}}\qquad\quad\checkmark$

Answer:

The mass is 1.68 grams

_______________________

I Hope this helps, greetings ... Dexteright02! =)

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Mercury has a specific gravity of 13.6. how many milliliters of mercury have a mass of 0.35 kg

Answers

The formula for specific gravity is:

$Specific gravity = (\rho _(substance))/(\rho _(water))$

where $\rho _(substance)$ is the density of the substance and $\rho _(water)$ is the density of water.

The density of water, $\rho _(water)$ = $1 g/mL$

Substituting the values in above formula we get,

$13.6 = (\rho _(substance))/(1)$

$\rho _(substance) = 13.6 g/mL$

The formula of density is:

$density = (mass)/(volume)$

The density of mercury is $13.6 g/mL$

The mass of mercury is $0.35 kg = 0.35 kg * 1000 (g)/(kg) = 350 g$

Substituting the values in density formula:

$13.6 g/mL = (350 g)/(volume)$

$volume = (350 g)/(13.6 g/mL) = 25.73 mL$

The amount, in milliliters, of mercury that will have a mass of 0.35 kg would be 25.74 mL.

If the specific gravity of mercury is 13.6, the density can be obtained such that:

Density of mercury = specific gravity of mercury/density of water

The density of water is 1 g/mL. Thus:

Density of mercury = 13.6/1

= 13.6 g/mL

Also; density = mass/volume

volume = mass/density

= 350/13.6

= 25.74 mL

Thus, the number of milliliters of mercury that will have a mass of 0.35 kg would be 25.74.

More on density can be found here: brainly.com/question/14940265?referrer=searchResults

Which two factors must be equal when a chemical reaction reaches equilibrium?(1) the concentration of the reactants and the concentration of the products
(2) the number of reactant particles and the number of product particles
(3) the rate of the forward reaction and the rate of the reverse reaction
(4) the mass of the reactants and the mass of the products

Answers

The correct answer is option 3. Equilibrium is achieved in a chemical reaction when the rate of the forward reaction is the same for the rate of the backward reaction and when the reaction has stopped.

Which best describes the particles in a gas when the temperature rises from 23 °C to 46 °C? A. The average energy doubles.

B. The average energy increases.

C. The average velocity of the particles increases by a factor of sqrt 2 .

D. The average energy remains constant but the velocity of some particles increases

Answers

I think the correct answer is b. Temperature is proportional to the average kinetic energy so when temperarure rises so will the average kinetic energy. I hope this helps. Let me know if anything is unclear.

Final answer:

When the temperature of a gas rises, the average energy of the particles increases. According to the Kinetic Molecular Theory, kinetic energy is proportional to its temperature. However, a rise in temperature doesn't directly double the energy.

Explanation:

The behavior of particles in a gas is very much affected by temperature changes. When the temperature of a gas increases, so too does the energy that the gas's particles have. This is defined by the Kinetic Molecular Theory, which states that the kinetic energy of a gas is proportional to its temperature. Therefore, when the temperature of a gas rises from 23°C to 46°C, the average energy of the particles increases. However, it doesn't double as an increase in temperature is not responsible for directly doubling the energy. Additionally, this increase in energy results in an increase in the velocity of the particles, but not necessarily by a factor of sqrt(2).

Learn more about Kinetic Molecular Theory here:

brainly.com/question/33444865

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A sample of hydrogen gas, has a volume of 8.56 L at a temperature 0oC and pressure of 1.5 atm. Calculate the number of moles of hydrogen present in this gas sample ( Assume that the gas behave ideally)

Answers

According to ideal gas law, there are 0.00565 number of moles of hydrogen present in the gas sample .

What is ideal gas law?

The ideal gas law is a equation which is applicable in a hypothetical state of an ideal gas.It is a combination of Boyle's law, Charle's law,Avogadro's law and Gay-Lussac's law . It is given as, PV=nRT where R= gas constant whose value is 8.314.The law has several limitations.Ideal gas law was proposed by Benoit Paul Emile Clapeyron in year 1834.It is a thermodynamic equation which has wide applications.

Gases which obey ideal gas law are difficult to exist.

Substituting the values as, P=1.5 atmospheres, V=8.56 L, R=8.314 ,T=0°C=273 K that is , n=PV/RT=1.5×8.56/8.314×273=0.00565 moles.

Thus, there are 0.00565 moles of hydrogen present in the gas sample .

Learn more about ideal gas law,here:

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p = 1.5atm ≈ 1519.88hPa
V = 8.56L
R = 83.1 [hPa*L] / [mol*K]
T = 0°C =273K

pV = nRT |:RT

n = pV / RT

n = [1519.88hPa*8.56L] / [83.1 [hPa*L] / [mol*K] * 273K]
n ≈ 0.57mol

What volume of a 2.5 M stock solution of acetic acid (HC2H3O2) is required to prepare 100.0 milliliters of a 0.50 M acetic acid solution?

Answers

Mi * Vi = Mf * Vf

2.5 * Vi = 0.50 * 100.0

2.5 Vi = 50

Vi = 50 / 2.5

Vi = 20 mL

hope this helps!

Answer:

20 milliliters

Explanation:

I don't cap

Why do ionic compounds have high melitng points??

Answers

An ionic compound is arranged in a organised lattice structre that allows for the greatest electrostatic attraction between the opposite charged atoms and the lesser electrostatic repulsion between the same atoms, where the atoms are as closely packed as possible. So the amount of energy (in form of heat) needed to break the electrostatic attraction between the atoms, so this means that ionic compounds have very high melting points.

because of its bondsIonic bonds are very strong - a lot of energy is needed to break them. So ionic compounds have high melting and boiling points.

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